To determine whether iodine pentachloride (ICl5) is polar or nonpolar, we need to look at its molecular geometry and the electronegativity of the atoms involved.
ICl5 has a square pyramidal shape due to its five chlorine atoms around a central iodine atom. The iodine atom is less electronegative than chlorine, creating polar covalent bonds between I and Cl. While the individual bond dipoles are polar, the overall molecule’s polarity depends on the symmetry of the shape.
In the case of ICl5, the square pyramidal geometry results in an asymmetrical distribution of charge. This means that the dipoles do not cancel out completely. Therefore, ICl5 has a net dipole moment, classifying it as a polar molecule.
In summary, ICl5 is polar due to its molecular shape and the presence of polar bonds that do not cancel out.